Permanganate Oxidation of Oxalic Acid

2MnO4− + 5C2O42− + 16H+ → 2Mn2+ + 10CO2 + 8H2O

Übersicht

Permanganate oxidizes oxalate to CO₂ while Mn(VII) is reduced to Mn(II). This reaction is autocatalytic: the Mn²⁺ product catalyzes the reaction, so it starts slowly and accelerates dramatically. The purple permanganate is decolorized as the reaction proceeds. It is a classic redox titration used in analytical chemistry.

Teilnehmer

Rolle Substanz Koeffizient Zustand
Reaktant Oxalic Acid C₂H₂O₄ 5 (aq)
Produkt Water H₂O 8 (l)
Produkt Carbon Dioxide CO₂ 10 (g)

Alltägliches Beispiel

This reaction demonstrates autocatalysis: the first drops of permanganate decolorize slowly, but later drops disappear almost instantly.

Industrielle Bedeutung

Permanganate-oxalate titration is used to standardize permanganate solutions and as a teaching example of autocatalytic kinetics.

Eigenschaften

Typ
Redox
Reversibel
Nein
Energie
Exotherm
ΔH
-489,0 kJ/mol

Verwandte Reaktionen

Iron(II) to Iron(III) Oxidation by Oxygen Bleaching with Sodium Hypochlorite Copper Reduction of Silver Ion Aqua Regia Dissolving Gold Cerium(IV) Reduction by Iron(II) Chlorine Oxidation of Bromide Copper Oxidation by Nitric Acid Hypochlorite Oxidation of Hydrogen Peroxide Hydrogen Peroxide as Oxidizing Agent (Acidic) Displacement of Hydrogen from Acid by Magnesium

Frequently Asked Questions

What is the equation for Permanganate Oxidation of Oxalic Acid?
The balanced equation is: 2MnO₄⁻ + 5C₂O₄²⁻ + 16H⁺ → 2Mn²⁺ + 10CO₂ + 8H₂O.
What type of reaction is Permanganate Oxidation of Oxalic Acid?
Permanganate Oxidation of Oxalic Acid is a redox reaction.
Is Permanganate Oxidation of Oxalic Acid exothermic or endothermic?
Permanganate Oxidation of Oxalic Acid is exothermic (releases energy). The enthalpy change (ΔH) is -489.0 kJ/mol.